6D.5

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605324529
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Joined: Mon Jun 17, 2019 7:24 am

6D.5

Postby 605324529 » Mon Jan 20, 2020 6:54 pm

Calculate the pH, pOH, and percentage protonation of sol- ute in each of the following aqueous solutions: (a) 0.057 m NH3(aq)
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Emily Chirila 2E
Posts: 112
Joined: Sat Jul 20, 2019 12:16 am

Re: 6D.5

Postby Emily Chirila 2E » Mon Jan 20, 2020 7:56 pm

You need to make an ice table for the reaction of NH3 reacting with H2O. Once you solve for the equilibrium concentration of OH-, you can find pOH (pOH= -log[OH-]). Then you can convert pOH to pH (pH + pOH = 14). Percentage protonation is calculated by doing ([NH4+]/[NH3]initial) x100%
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DesireBrown1J
Posts: 98
Joined: Wed Sep 18, 2019 12:18 am

Re: 6D.5

Postby DesireBrown1J » Thu Jan 23, 2020 10:16 pm

Emily Chirila 2E wrote:You need to make an ice table for the reaction of NH3 reacting with H2O. Once you solve for the equilibrium concentration of OH-, you can find pOH (pOH= -log[OH-]). Then you can convert pOH to pH (pH + pOH = 14). Percentage protonation is calculated by doing ([NH4+]/[NH3]initial) x100%



How are we supposed to solve for x in the ICE table if we do not know what Kb is?
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Olivia Smith 2E
Posts: 101
Joined: Wed Sep 30, 2020 9:43 pm

Re: 6D.5

Postby Olivia Smith 2E » Thu Jan 28, 2021 7:30 pm

There is a table with all of the values in the textbook. Idk what the actual place it is but if you scroll up a bit you should see all of the tables with the Kb values
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